91Ó°ÊÓ

How would you select an indicator for a particular acid-base titration?

Would the \(\mathrm{pH}\) at the equivalence point of a titration of a weak acid with a strong base be less than, equal to, or greater than 7.0\(?\)

Name an indicator you might use to titrate ammonia with hydrochloric acid.

The \(K_{a}\) of nitrous acid, \(\mathrm{HNO}_{2},\) is \(6.76 \times 10^{-4} .\) Write the equation describing the equilibrium established when \(\mathrm{HNO}_{2}\) reacts with \(\mathrm{NH}_{3} .\) Use unequal arrows to indicate whether reactants or products are favored.

\(\begin{array}{l}{\text { a. What is the relationship between the }} \\\ {\text { strength of an acid and the strength of }} \\ {\text { its conjugate base? }} \\ {\text { b. What is the realtionship between the }} \\ {\text { strength of a base and the strenght of }} \\ {\text { its conjugate acid? }}\end{array}\)

Propanoic acid, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{COOH},\) is a weak acid. Write the expression defining its acid-ionization constant.

Place the following acids in order of increasing strength: \begin{equation} \begin{array}{l}{\text { a. valeric acid, } K_{a}=1.5 \times 10^{-5}} \\\ {\text { b. glutaric acid, } K_{a}=3.4 \times 10^{-4}} \\ {\text { c. hypoobromous acid, } K_{a}=2.5 \times 10^{-9}} \\ {\text { d. acetylsalicylic acid (aspirin), }} \\ {K_{a}=3.3 \times 10^{-4}}\end{array} \end{equation}

What are the components of a buffer solution? Give an example.

How much \(\mathrm{HCl}\) would you need to dissolve in 1.0 \(\mathrm{L}\) of water so that \(\left[\mathrm{OH}^{-}\right]=\) \(6.0 \times 10^{-12} \mathrm{M} ?\)

If 0.150 mol of \(\mathrm{KOH}\) is dissolved in 500 \(\mathrm{mL}\) of water, what are \(\left[\mathrm{OH}^{-}\right]\) and \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) ?